Rate of Reactions

Rate of Reaction

A measure of how fast a reaction occurs, often expressed in units of concentration change over time, such as mol/(L·s).

Collision Theory

A theory that states that chemical reactions occur when reactant particles collide with sufficient energy and proper orientation.

Potential Energy Diagram

A graphical representation of the energy changes during a chemical reaction, showing the energy of reactants, products, and the activated complex.

Activation Energy (Ea)

The minimum amount of energy required for a reaction to occur, represented in a potential energy diagram.

Enthalpy Change (ΔH)

The difference in energy between reactants and products in a chemical reaction, indicating whether a reaction is endothermic or exothermic.

Reaction Mechanism

The detailed sequence of elementary steps that occur in a chemical reaction.

Reactant

A substance that undergoes a chemical change in a reaction.

Intermediate

A species formed during the reaction but not present in the final products.

Catalyst

A substance that increases the rate of a reaction without being consumed in the process.

Product

The substances formed as a result of a chemical reaction.

Rate Determining Step

The slowest step in a reaction mechanism that determines the overall rate of the reaction.

Overall Reaction

The net equation that summarizes the entire reaction mechanism, showing the reactants and products.

Rate Law

An equation that relates the rate of a reaction to the concentration of the reactants with respect to their orders.

Rate Constant (k)

A proportionality constant in the rate law that is specific for a given reaction at a given temperature.

Reaction Intermediates

Species that are formed and consumed during the reaction mechanism but do not appear in the overall equation.

Chemical Kinetics

The study of the rates of chemical reactions and the factors affecting them.